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Question

Which of the following solutions will have pH equal to 1.0?

A
55 mL of M10 HCl + 45 mL of M10 NaOH
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B
50 mL of M5 HCl + 50 mL of M5 NaOH
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C
75 mL of M5 HCl + 25 mL of M5 NaOH
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D
None of the above
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Solution

The correct option is C 75 mL of M5 HCl + 25 mL of M5 NaOH

We need to calculate the resulting molar concentration of H+ ions to determine the resulting pH of solutions.
Here n-factor of NaOH and HCl is 1 . So Molarity and Normality are equal.
Formula used is:
Mmix=M1V1M2V2V1+V2 if M1V1>M2V2
Option A: (0.1×55)>(0.1×45) Nmix=(0.1×55)(0.1×45)100=0.01pH=log(0.01)=2×log(10)=2

Option B: Since the concentration and volume of both NaOH and HCl is equal. It forms a neutral solution of pH=7

Option C: (0.2×75)>(0.2×25)
Nmix=(0.2×75)(0.2×25)100=0.1pH=log(0.1)=log(10)=1

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